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(A) The total pressure of air over water is $10\ atm$.The partial pressure of nitrogen is $P_{N_2} = \frac{79}{100} 	imes 10\ atm = 7.9\ atm = 7.9

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(A) The total pressure of air over water is $10\ atm$.The partial pressure of nitrogen is $P_{N_2} = \frac{79}{100} 	imes 10\ atm = 7.9\ atm = 7.9 	imes 760\ mm\ Hg = 6004\ mm\ Hg$.The partial pressure of oxygen is $P_{O_2} = \frac{20}{100} 	imes 10\ atm = 2.0\ atm = 2.0 	imes 760\ mm\ Hg = 1520\ mm\ Hg$.According to Henry's law,$P = K_H 	imes X$,where $X$ is the mole fraction of the gas in the solution.$X_{N_2} = \frac{P_{N_2}}{K_H(N_2)} = \frac{6004}{6.51 	imes 10^7} = 9.22 	imes 10^{-5}$.$X_{O_2} = \frac{P_{O_2}}{K_H(O_2)} = \frac{1520}{3.30 	imes 10^7} = 4.60 	imes 10^{-5}$.The mole ratio of dissolved gases is $\frac{X_{O_2}}{X_{N_2}} = \frac{4.60 	imes 10^{-5}}{9.22 	imes 10^{-5}} \approx 0.5 = \frac{1}{2}$.

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